In a chemical reaction you collect 1000 ml of hydrogen gas at stp how many moles of hydrogen gas did you collect 0.02 0.04 0.004 0.002

Option B = 0.04 mol

Explanation:

We were given the following:

Pressure = 1 atm (We know this because it was stated that the gas is at STP).

Volume = 1000ml = 1L (Converting to L by diving by 1000)

Temperature = 273.15k (We know this because it was stated that the gas is at STP).

We are to calculate the number of moles, n collected.

The Ideal Gas Equation relates all of these variables;

pV=nRT

where R = gas constant = 0.08206 L atm / K mol

making n subject of interest, we have;

n=pV / RT

Substituting the values of the variables and solving for n;

n = (1 * 1 ) / (0.08206 * 273.15)

n = 0.0446 mol

Approximately, n = 0.04 mol

answer: the value of enthalpy change will be -152.80 kj.

solution:

pressure = 1atm , temperature = = 298 k

given that pressure and temperature are same in both gases , the number of moles of both gases can be determined by the ideal gas equation.

according to reaction 3 moles no are reacting with 1 mol of ,then 0.49 mol of no will react with moles of ozone that is 0.16 moles of ozone. since, no is limiting reagent and is an excessive reagent.

enthalpy change for the reaction between the given volumes of the gases is :