1.Balance the chemical equation given below, and calculate the volume of nitroge

Question

1.Balance the chemical equation given below, and calculate the volume of nitrogen monoxide gas produced when 8.00 g of ammonia is reacted with 12.0 g of oxygen at 25°C? The density of nitrogen monoxide at 25°C is 1.23 g/L. _____ NH3(g) + _____ O2(g) ______ NO(g) + _____ H2O(l)

2.Given three cylinders containing O2 gas at the same volume and pressure. Cylinder A is at -15°C, cylinder B is at -5°F, cylinder C is at 255 K. Which cylinder contains the largest mass of oxygen?

3.The following reaction is used to generate hydrogen gas in the laboratory. If 243 mL of gas is collected at 25°C and has a total pressure of 745 mm Hg, what mass of hydrogen is produced? A possibly useful table of water vapor pressures is provided below.

4.How many grams of calcium chloride are needed to produce 1.50 g of potassium chloride?
CaCl2(aq) + K2CO3(aq) 2 KCl(aq) + CaCO3(aq)

Explanation / Answer

NH3 + O2 = NO + H2O

the balance

4 NH3 + 5 O2 = 4 NO + 6 H2O

mol of NH3 = mass/MW = 8/17 = 0.470588

mol of O2 = mass/MW = 12/32 = 0.375

ratio is 4:5 so

0.375 mol of O2 --> 4/5*0.375 = 0.3 mol of NO

mass = mol*MW = 0.3*30 =9 g of NO

V = m/D = 9/1.23

V = 7.317073 mL

NOTE Consider posting multiple questions in mutliple set of Q&A.

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