Answer:
The fertilizer ammonium sulfate, (NH4)2SO4, is prepared by the reaction of ammonia, NH3, with sulfuric acid: 2 NH3 (g) + H2SO4 (aq) (NH4)2SO4 (aq)
How many moles of ammonium sulfate are produced if 1.50 moles of ammonia react completely at STP? Answer: The balanced equation indicates that 2 moles of NH3 react to produce 1 mole of (NH4)2SO4.
1.50 moles NH3 x 1 mol (NH4)2SO4 = 0.750 moles (NH4)2SO4
Explanation:
Answer:
Q < K for both reactions. Both are spontaneous at those concentrations of substrate and product.
Explanation:
Hello,
In this case, the undergoing chemical reactions with their proper Gibbs free energy of reaction are:


The cellular concentrations are as follows: [A] = 0.050 mM, [B] = 4.0 mM, [C] = 0.060 mM and [D] = 0.010 mM.
For each case, the reaction quotient is:

A typical temperature at a cell is about 30°C, in such a way, the equilibrium constants are:

Therefore, Q < K for both reactions. Both are spontaneous at those concentrations of substrate and product.
Best regards.
I think the answer is D in my opinion
Honestly I don’t even know