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URGENT CAN SOMEONE ANSWER THIS QUESTION AND SHOW THEIR WORK PLEASE! How many moles of ammonia (NH) can be produced from the reaction of 4.0 liters of hydrogen at 50.0°C and 1.2atm of pressure with excess nitrogen?

User Sadlil
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The balanced chemical equation for the reaction of hydrogen (H2) with nitrogen (N2) to produce ammonia (NH3) is:

N2 + 3H2 → 2NH3

To calculate the number of moles of ammonia produced from the given amount of hydrogen, we need to use the ideal gas law to determine the number of moles of hydrogen present in the reaction:

PV = nRT

where P is the pressure, V is the volume, n is the number of moles, R is the gas constant, and T is the temperature in Kelvin.

First, we need to convert the given temperature of 50.0°C to Kelvin:

T = 50.0°C + 273.15 = 323.15 K

Next, we can use the ideal gas law to calculate the number of moles of hydrogen:

n = PV/RT = (1.2 atm)(4.0 L)/(0.08206 L·atm/mol·K)(323.15 K) = 0.181 mol

According to the balanced chemical equation, 3 moles of hydrogen react to produce 2 moles of ammonia. Therefore, the number of moles of ammonia produced is:

0.181 mol H2 × (2 mol NH3 / 3 mol H2) = 0.121 mol NH3

So 0.121 moles of ammonia can be produced from the given amount of hydrogen.

User Hua Zhang
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