A 22.0 g sample of propane is burned in a bomb calorimeter that contains 300. g of water. If the temperature change is 18.5∘C and the heat capacity of the calorimeter is 824 J∘C, how much heat was released by the combustion of the propane sample? Assume the heat capacities of the reaction products are negligible compared to that of the water and the calorimeter. The specific heat capacity of water is 4.184 J g∘C. Your answer should have three significant figures. Enter the amount of heat released as a positive quantity. Provide your answer below:
A 1.00 g sample of hydrazine (N2H4) is burned in a bomb calorimeter containing 1200. g of water that experiences a temperature change of 3.54∘C. If the heat capacity of the calorimeter is 840. JC, what is the heat of combustion for the sample? The specific heat capacity of water is 4.184 J g∘C. Your answer should have three significant figures. Provide your answer below: kJ
6.45 g of C6H12O6 is burned in a bomb calorimeter containing 950. g of water and the temperature goes from 35.0∘C to 42.3∘C. If the bomb has a heat capacity of 933 J∘C, what is the value for q of the reaction? The specific heat capacity of water is 4.184 J g∘C. Your answer should have three significant figures. When reporting your answer in scientific notation format, use the multiplication symbol, ×, not the letter x. Do not include a comma in your answer. Provide your answer below:
A 1.0 g sample of C8H18 is burned in a bomb calorimeter with a heat capacity of 837 J∘C that holds 1,200 g of water at 25⋅0∘C. After the reaction, the final temperature of the water is 33.2∘C. What is the value of q for the combustion of C8 H18, in kJ ? The specific heat capacity of water is 4.184 Jng∘C. Your answer should have two significant figures. Provide your answer below:
A 1.00 g sample of octane (C8H18) is burned in a bomb calorimeter with a heat capacity of 837 J∘C that holds 1200. g of water at 25.0∘C. After the reaction, the final temperature of the water is 33.2∘C. Calculate the heat of combustion for 1.00 mol of octane. Use 4.184 J g∘C for the specific heat capacity of water. Your answer should have three significant figures.
A sample of water cools down from 89.7∘C to 43.2∘C by releasing 1.47×103 kJ of heat. What is the mass of water in this sample in grams? Report the answer with three significant figures. Report the answer in scientific notation. Use 4.184 J g∘C for the specific heat of water. Provide your answer below: g
A 45.0 g piece of metal with specific heat 0.450 J g∘C and at 115∘C is placed in 200. g of water at 25.0∘C. What will be the final temperature of the water? Select the correct answer below: 2.10∘C 29.8∘C 88.4∘C 27.1∘C
A 1.50 kg copper pipe at 800.0∘C is immersed into a 20.0∘C bucket of water with a mass of 5.00 kg. What is the final temperature of the copper-water mixture if the specific heat of copper is 0.386 J g∘C and the specific heat of water is 4.184 J g∘C ? Round your answer to one decimal place Provide your answer below: ∘C
A mass of copper at 25.50∘C is placed in a calorimeter filled with 236 g of hot water at 38.00∘C. The final temperature of the water is 36.90∘C. What is the mass of copper in grams? Your answer should have three significant figures (Round to a whole number). Use 0.385 J g∘C for the specific heat of copper. Use 4.184 J g∘C for the specific heat of water. Provide your answer below:
Use the periodic table to answer the following question: If 3.60 g of NaHSO4 react, what is the change in enthalpy for the reaction, in kilojoules? 2 NaHSO4(s) ⟶ Na2SO4(s) + H2O(g) + SO3(g) ΔH = −231.3 kJ Include a negative sign, if appropriate. Do not include units in your response. Round your answer to two decimal places. Include a negative sign if appropriate. Provide your answer below: kJ
When 2.16 g of H2 reacts with excess O2 by the following equation, 258 kJ of heat are released. What is the change of enthalpy associated with the reaction of 1.00 mol of hydrogen gas? 2 H2 + O2 ⟶ 2 H2O Round your answer to the nearest whole number. Include a negative sign if appropriate. Provide your answer below: kJ/mol
If 1.48 g of Cl2 reacts with excess P, what is the total change in enthalpy in kilojoules? 2 P + 5 Cl2 ⟶ 2 PCl5 ΔH = −886 kJ Round your answer to three significant figures. Include a negative sign if appropriate. Provide your answer below:
What is the change in enthalpy associated with the combustion of 530 g of methane (CH4) ? When reporting your answer in scientific notation format, use the multiplication symbol, ×, not the letter x. Your answer should have two significant figures. Use −890.8 kJ/mol for the molar heat of combustion of methane. Provide your answer below: kJ
Given that 2S(s) + 3O2(g) → 2SO3(g) has an enthalpy change of −790.4 kJ 2SO2(g) + O2(g) → 2SO3(g) has an enthalpy change of −198.2 kJ What is the heat of formation of SO2 in kilojoules? S(s) + O2(g) → SO2(g)Your answer should have four significant figures. Provide your answer below: kJ
NH3(g) + HCl(g) ⟶ NH4Cl(s) Given the standard enthalpies of formation (below), calculate the enthalpy change for the reaction in kilojoules. NH3(g) ΔHf∘ = −46.1 kJ mol HCl(g) ΔHf∘ = −92.3 kJ mol NH4Cl(s) ΔHf∘ = −314.4 kJ mol Your answer should have three significant figures. Provide your answer below: kJ
If the heat of formation for CO2 is −393.5 kJ mol, what is the change in enthalpy when 5.00 g of CO2 are formed? Your answer should have three significant figures. (Round your answer to first decimal place). Provide your answer below: kJ
The standard heat of formation for NO2 is 33.2 kJ mol. How much energy is required to form 100.0 g of NO2 from its respective elements in kilojoules? Your answer should have three significant figures. (Round your answer to one decimal place). Provide your answer below: kJ
Consider the reaction described by the following chemical equation. 2 Ag2S(s) + 2 H2O(l) ⟶ 4 Ag(s) + 2 H2S(g) + O2(g) ΔHrxn∘ = 595.5 kJ mol The change in enthalpy for this reaction can be determined theoretically by using the standard enthalpies of formation for the species involved. ΔHrxn∘ = ∑nΔHf products ∘−∑nΔHf reactants ∘ What is the value for the standard enthalpy of formation for Ag(s) that would be used in the equation above? Provide your answer below: kJ/mol
Consider the following thermochemical equations. PCl5(s) → PCl3(g) + Cl2(g) ΔHrxn∘ = 87.9 kJ mol 2P(s) + 3Cl2(g) → 2PCl3(g) ΔHrxn∘ = −574 kJ mol Using this data, determine the heat of formation for PCl5. Your answer should have three significant figures. Provide your answer below: kJ/mol
Given the following equations, determine the standard enthalpy of formation (ΔHf∘) for one mole of ICl3(g). I2(g) + 3 Cl2(g) ⟶ 2 ICl3(g) ΔH298∘ = −214 kJ I2(s) ⟶ I2(g) ΔH298∘ = 38 kJ Note that iodine (I2) is a solid at standard conditions. Your answer should have two significant figures. Provide your answer below: kJ