Oxygen gas produced : 0.7 g
<h3>Further explanation</h3>
Given
10.0 grams HgO
9.3 grams Hg
Required
Oxygen gas produced
Solution
Reaction⇒Decomposition
2HgO(s)⇒2Hg(l)+O₂(g)
Conservation of mass applies to a closed system, where the masses before and after the reaction are the same
mass of reactants = mass of products
mass HgO = mass Hg + mass O₂
10 g = 9.3 g + mass O₂
mass O₂ = 0.7 g
Answer:
See detailed explanation.
Explanation:
Hello!
i. In this case, since the given chemical reaction is exothermic due to the negative change in the enthalpy of reaction, we infer that according to the mentioned principle, by lowering the temperature the reaction will shift rightwards and therefore the yield is increased; thus, you need a lower temperature than the specified.
ii. In this case, since the reaction has less moles at the products side, according to the mentioned principle it'd be necessary to rise the pressure in order to increase the yield, since the increase of pressure favors the reaction side with the fewest number of moles.
Best regards!
Answer:
A Chemical equation is balanced if the reactants side of the chemical reaction has the same number total of atoms of elements as the products side of the chemical equation. While a Chemical equation is unbalanced if the reactants side of the chemical reaction has a different number total of atoms of elements as the products side of the chemical equation
Explanation:
Self explanatory
Acids have hydronium ions and when dissolved in water, bases produce hydroxide ions. Hope this helps.
