When solid (NH4)(NH2CO2)(NH4)(NH2CO2) is introduced into and evacuated flask at 25∘C25∘C, the total pressure of gas at equilibrium is 0.30.3 atm. What is the value of Kpat25∘CKpat25∘C?

Kp = 0.004  = 4*10^-3

Explanation:

Step 1: Data given

Temperature = 25.0 °C

the total pressure of gas at equilibrium is 0.30 atm

Step 2: The balanced equation

NH4(NH2CO2)(s) ⇆ 2NH3(g) + CO2(g)

For 1 mol NH4(NH2CO2) we have 2 moles NH3 and 1 mol CO2

Step 3: The total pressure

Total pressure = pNH3 + pCO2

Total pressure = 2X + X

Total pressure = 3X = 0.30

X = 0.10

Step 4: The partial pressures

pNH3 = 2X = 2*0.10 = 0.20 atm

pCO2 = X = 0.10 atm

Step 5: Calculate Kp

Kp = (pNH3)²*(pCO2)

Kp = (0.20²)*0.10

Kp = 0.004  = 4*10^-3

its first and third is your answer i did the qustion the fourth isnt right