How man Liters are there in 450 grams of NH3 gas at STP?

When using mass values from the periodic table round to 2 decimal places. EX: H-1.008 g ----> 1.01 g

We use the ideal gas formula, with the constant R = 0.082 l atm / K mol. First, we calculate the number of moles of NH3 (we obtain the mass of 1 mol from the atomic weights of the elements of the periodic table).The STP conditions are : 1 atm pressure and 273 K temperature. Solve for the formula, V (volume):

Weight 1 mol NH3= Weight N + (Weight H)x3= 14,01 g + 3 x 1,01 g=17,04 g/mol

17,04 g ---1 mol NH3

450 g--x= (450 g x 1 mol NH3)/17,04g= 26,41 mol NH3

PV=nRT ---> V= (nRT)/P

V=(26,41 mol x 0.082 l atm / K mol x 273 K)/ 1 atm

V=591, 18 L

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How man Liters are there in 450 grams of NH3 gas at STP? When using mass values from the periodic table round to 2 decimal places. EX: H-1.008 g ----> 1.01 g

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How man Liters are there in 450 grams of NH3 gas at STP?

When using mass values from the periodic table round to 2 decimal places. EX: H-1.008 g ----> 1.01 g