1)how many molecules of water are needed to produce 6 molecules of C6H12O6 according to the equation 6CO2(G)+6H2O(L)+energy TO C6H12O6(S)+6O2(G)?
2)how many mole of oxygen gas are produce when 6 mol of CO2 are consumed in the process of photosynthesis(see above question for the equation)
3)H2(G)+Cl2(g) to 2HCl(g)if 2 mol of H gas are mixed with 4 mol of Cl gas, how many moles of HCl will be produced?
1) According to the balanced chemical equation:
6CO2(G) + 6H2O(L) + energy → C6H12O6(S) + 6O2(G)
The stoichiometry of the equation tells us that for every 6 molecules of CO2 consumed, 6 molecules of H2O are also consumed to produce 1 molecule of C6H12O6. Therefore, in order to produce 6 molecules of C6H12O6, we would need 6 molecules of H2O.
2) Again, according to the balanced chemical equation:
6CO2(G) + 6H2O(L) + energy → C6H12O6(S) + 6O2(G)
The stoichiometry of the equation tells us that for every 6 molecules of CO2 consumed, 6 molecules of O2 are produced. Since 6 moles of CO2 are consumed, we can infer that 6 moles of O2 are produced as well.
3) According to the balanced chemical equation:
H2(G) + Cl2(g) → 2HCl(g)
The stoichiometry of the equation tells us that 1 mole of H2 gas reacts with 1 mole of Cl2 gas to produce 2 moles of HCl. Therefore, if we have 2 moles of H2 gas and 4 moles of Cl2 gas, all the H2 will be reacted, and the limiting reactant (Cl2) will determine the amount of HCl produced. Since the stoichiometry ratio is 1:1, we can conclude that 2 moles of HCl will be produced.
1) To find the number of molecules of water needed to produce 6 molecules of C6H12O6, we can use the balanced equation provided: 6CO2(G)+6H2O(L)+energy → C6H12O6(S)+6O2(G).
The coefficients in the equation represent the molar ratios, indicating the ratio of moles of each substance involved in the reaction. In this case, it shows that for every 6 moles of CO2 consumed, 6 moles of H2O are needed to produce 1 mole of C6H12O6.
Since we are given the number of molecules, we need to convert them to moles. One mole of any substance contains Avogadro's number (6.022 x 10^23) molecules. Therefore, 6 molecules is equal to 6/Avogadro's number moles.
Using the molar ratio from the balanced equation, we find that 6 moles of CO2 corresponds to 6 moles of H2O. Therefore, the number of moles of water needed is also 6/Avogadro's number.
2) To find the number of moles of oxygen gas produced when 6 moles of CO2 are consumed, we again refer to the balanced equation: 6CO2(G)+6H2O(L)+energy → C6H12O6(S)+6O2(G).
According to the equation, for every 6 moles of CO2 consumed, 6 moles of oxygen gas are produced. Therefore, the number of moles of oxygen gas produced is equal to the number of moles of CO2 consumed.
Given that 6 moles of CO2 are consumed, the number of moles of oxygen gas produced is also 6 moles.
3) The balanced equation for the reaction H2(G)+Cl2(g) → 2HCl(g) tells us that the ratio of moles of H2 to moles of HCl is 1:2.
In the given scenario, we have 2 moles of H2 and 4 moles of Cl2. In order to determine how many moles of HCl will be produced, we need to identify the limiting reactant, which is the reactant that will be consumed completely and determines the maximum amount of product that can be formed.
To do this, we compare the mole ratios of the reactants. From the balanced equation, we see that the ratio of moles of H2 to moles of HCl is 1:2, while the ratio of moles of Cl2 to moles of HCl is 1:1.
Since 2 moles of H2 would require 2 x 2 = 4 moles of HCl, it matches the number of moles of Cl2 available (4 moles). Therefore, 4 moles of HCl will be produced.
1. The equation tells you 6 molecules of water are needed to produce 6 molecules of C6H12O6.
2. The equation tells you that 6 moles of O2 are produced for 6 moles CO2 consumed.
3. H2 + Cl2 ==> 2HCl
2 moles H2 gas will react with 2 moles Cl2 gas to produce 4 moles HCl gas. Two moles of the Cl2 gas will go un-reacted.