Consider the formation of nitrogen dioxide from nitric oxide and oxygen: 2NO(g) + O2(g) → 2NO2(g) If 6.23 L of NO is combined with excess O2 at STP, what is the volume in liters of the NO2 produced? Round your answer to 3 significant digits. L ×10
If 119.3 g of PCl5 are formed from the reaction of 61.3 g Cl2 with excess PCl3, what is the percent yield? PCl3(g) + Cl2(g) → PCl5(g) 66.3% 48.6% 57.3% 94.6% 51.3%
Germanium forms a substitutional solid solution with silicon. Compute the weight percent of germanium that must be added to silicon to yield an alloy that contains 2.74×1021 Ge atoms per cubic centimeter. The densities of pure Ge and Si are 5.32 and 2.33 g/cm3, respectively. The atomic weights for germanium and silicon are 72.64 and 28.09 g/mol, respectively. wt%
If 5.0 g of H2 are reacted with excess CO, how many grams of CH3 OH are produced, based on a yield of 86% ? CO(g) + 2H2(g) → CH3OH(l)
The "maximum sustainable yield" of a resource (that determines total allowable catch) is usually calculated to maintain the population at % of the environment's carrying capacity for that resource. 5 10 25 50 90
Determine the molarity of a solution formed by dissolving 97.7 g LiBr (molar mass = 86.85 g/mol) in enough water to yield 750.0 mL of solution. 1.50 M 1.18 M 2.30 M 0.768 M 0.130 M
Percent yield is the percent ratio of actual yield to the theoretical yield. It is calculated to be the experimental yield divided by theoretical yield multiplied by 100%. % yield = actual yield theoretical yield ×% Consider the following reaction, if the percent yield of BaCO3(s) is 84.98 %, and theoretical yield is 0.63 g, what is the actual yield of BaCO3(s) ? Ba(NO3)2(aq) + Na2CO3(aq) ⟶ 2NaNO3(aq) + BaCO3(s)
How many moles are present in a 185. g sample of X(NO3)2. The molar mass of element X is 119.57 g/mol. Use the correct number of significant figures in your answer. Do not enter the unit.
A 4.60 mol sample of solid A was placed in a sealed 1.00 L container and allowed to decompose into gaseous B and C. The concentration of B steadily increased until it reached 1.20 M, where it remained constant. A(s) ⇌ B(g) + C(g) Then, the container volume was doubled and equilibrium was re-established. How many moles of A remain? moles of A: mol
At a certain temperature the vapor pressure of pure chloroform (CHCl3) is measured to be 310. torr. Suppose a solution is prepared by mixing 115. g of chloroform and 119. g of acetyl bromide (CH3COBr). Calculate the partial pressure of chloroform vapor above this solution. Be sure your answer has the correct number of significant digits. Note for advanced students: you may assume the solution is ideal. torr ×10
Nitrogen gas can be prepared by passing ammonia over copper(II) oxide, and the other products are copper metal and water vapor. If a sample containing 5.78 moles of NH3 is reacted with excess copper(II) oxide, how many grams of N2 will be formed?
Determine the molarity of a solution formed by dissolving 97.7 g LiBr (molar mass = 86.85 g/mol) in enough water to yield 750.0 mL of solution. 1.50 M 1.18 M 2.30 M 0.768 M 0.130 M
Calculate the percent yield of a reaction if 35.00 g of Fe2O3 react with excess AI and the actual yield is 22.65 g of Fe. Hint: You need to find the theoretical yield first Fe2O3(s) + 2Al(s) → Al2O3(s) + 2Fe(s) 60.17% 40.56% 64.71 46.26% 92.52%
Methyl bromide is a highly toxic gas used as a fumigant for soil. It can be produced by reacting methanol with hydrogen bromide in a substitution reaction as follows: CH3OH(l) + HBr(g) → CH3Br(g) + H2O(l) If the standard heat of formation of methyl bromide gas is −35.5 kJ/mol, what is the enthalpy of the above substitution reaction? Select one: a. −118.4 kJ b. −45.9 kJ c. −1.8 kJ d. −239.9 kJ