True or False
OP already did it - CONGRATS!!
here are the steps 2 get the same ans:
(NH4)2 CO3 has 2x N, 8x H, 1x C and 3x O per molecule
so its molecular mass = 2x14 + 8x1 + 1x12 + 3x16
=28+8+12+48
=96g
of that 96g, 8x1=8g is due to Hydrogen
so by ratio n proportion, 1.00g will have 1x8/96 = 1/12g = 0.083g of H
Answer:
22.4 L methane reacts with 44.8L of oxygen to give 44.8L of CO
2 and 22.4 L of water
Explanation:
From the balanced reaction: One mole(or 1 molecule or 16 g) of CH
4
reacts with 2 moles (or 2 molecules or 64 g) of oxygen to give one mole (or 1 molecule or 44 g) of CO
2
and 2 mole (or 2 molecules or 36 g) of water.
For the gaseous system at STP:
22.4 L methane reacts with 44.8 L of oxygen to give 22.4 L of CO
2
and 44.8 L of water.
and 2 mole (or 2 molecules or 36 g) of water.
For the gaseous system at STP:
22.4 L methane reacts with 44.8 L of oxygen to give 22.4 L of CO
2
and 44.8 L of water.
b. Products are favored over reactants in the reaction.
c. Reactants are favored over products in the reaction.
d. All of the reactants have turned into products in the reaction.
If Keq equals 1, this means the reaction is at equilibrium and neither the reactants nor the products are favored. The concentrations of both remain constant over time.
When Keq = 1, it implies that the reaction is at equilibrium and neither the reactants nor the products are favored in the reaction. So, the correct answer to your question is option a: Products and reactants are equally favored in the reaction.
In this situation, the concentrations of products and reactants remain constant over time because the rate of the forward reaction equals the rate of the reverse reaction.
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For a chemical equilibrium, Keq = 1 indicates that neither reactants nor products are favored; rather, they are present in roughly equal amounts at equilibrium. So the correct answer is Option C.
If Keq = 1 for a chemical equilibrium, it means that products and reactants are equally favored in the reaction. In other words, neither the reactants nor the products are favored when the reaction reaches equilibrium. Equilibrium constants help us understand the extent to which a reaction occurs. When Keq is greater than 1, the concentration of products at equilibrium is greater than the concentration of reactants, suggesting a product-favored reaction. Conversely, when Keq is less than 1, the concentration of reactants is higher, indicating a reactant-favored reaction. When Keq is equal to 1, it implies that the concentrations of reactants and products are roughly equal at equilibrium, reflecting a state of balance in the chemical system.
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