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Ammonium nitrite decomposes to give off nitrogen gas and liquid water. How many grams of ammonium nitrite must have reacted if 2.58 L of gas was collected over water in a gas collecting tube at 21.0°C and 97.8 kPa?

Balanced equation:

Ans to 3:

(6 pts) Will the volume of nitrogen (from the previous problem) INCREASE, DECREASE or remain the SAME if... *Explain briefly*

...the experiment is done at significantly higher temperature?

B. ...the amount of ammonium nitrite was increased?

C.

...the experiment was not collected over water?

4. (10 pts) 900.0 mL of 3.00M phosphoric acid, H PO, reacts with 235 grams of iron (III) carbonate.

Balanced Equation: Fez(CO;) + 2H;PO4 - 2FePO4 + 3H20 + 3C02

a. Determine the limiting reactant. Show all work!

Ans to 4a:

b. How many milliters of carbon dioxide gas can be produced at 78°C at 45.5 psi pressure with 900.0 mL of 3.00M phosphoric acid and 235 grams of iron (III) carbonate?

PLEASE SOMEONE I NEED HELP WITH CHEMISTRY FAST no fake answers either please Ammonium nitrite decomposes to give off nitrogen gas and liquid water How

Answer :

70.0 L of CO2 gas can be produced at 78°C at 45.5 psi pressure with 900.0 mL of 3.00 M phosphoric acid and 235 grams of iron (III) carbonate.

Volume of nitrogen gas collected = 2.58 LPressure of nitrogen gas collected = 97.8 kPaTemperature of nitrogen gas collected = 21.0°CBalanced chemical equation:NH4NO2(s) → N2(g) + 2H2O(l)The volume of nitrogen (from the previous problem) will increase if the experiment is done at a significantly higher temperature. This is because with the increase in temperature, the kinetic energy of the gas molecules increases, and the volume increases.The volume of nitrogen will remain the same if the amount of ammonium nitrite was increased. This is because the volume of gas produced is directly proportional to the amount of ammonium nitrite used in the reaction.The experiment not collected over water will give incorrect results as the water vapor in the gas will also be collected along with nitrogen gas. This will increase the volume of the gas collected and thus lead to incorrect results.4. (a) Given,Molarity of H3PO4 = 3.00MMoles of H3PO4 = Molarity × Volume in liters= 3.00 × (900.0 mL/1000 mL/L)= 2.70 molesMoles of Fe2(CO3)3= Mass/Molar mass= 235 g/291.72 g/mol= 0.805 molesAccording to the balanced chemical equation,1 mole of Fe2(CO3)3 reacts with 2 moles of H3PO4Therefore, moles of H3PO4 required for complete reaction with Fe2(CO3)3= 0.805 mol/2= 0.4025 moles.Therefore, H3PO4 is the limiting reactant.4. (b) The balanced chemical equation is,Fe2(CO3)3 + 2H3PO4 → 2FePO4 + 3CO2 + 3H2OAccording to the balanced equation,1 mole of Fe2(CO3)3 produces 3 moles of CO2.

Therefore, 0.805 moles of Fe2(CO3)3 produces 3 × 0.805 = 2.415 moles of CO2.Volume of CO2 at STP = 2.415 × 22.4 L= 54.1 LBut the given conditions are not at STP. We need to use the ideal gas equation,PV = nRTR = 0.08206 L.atm/K.molP = 45.5 psi = 45.5/14.696 atm= 3.1 atmT = (78 + 273) K = 351 K.Volume of CO2 at given conditions= (2.415 mol × 0.08206 L.atm/K.mol × 351 K)/3.1 atm= 70.0 L.

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