32.7 g Zn
Explanation:
First convert the amount of gas into moles:
11.2 L H2 × (1 mol H2/22.4 L H2) = 0.500 mol H2
Then use the molar ratio to find the amount of zinc necessary to produce the amount of gas above:
0.500 mol H2 × (1 mol Zn/1 mol H2)
= 0.500 mol Zn
Now use the molar mass of zinc to find the number of grams of zinc for the reaction to occur:
0.500 mol Zn × (65.38 g Zn/1 mol Zn)
= 32.7 g Zn
If the experiment is not performed right,you can redo the experiment.
214.746049. I converted between grams Manganese
Answer:
c. the same as
Explanation:
for a closed system:
⇒ ΔS > 0.....irreversible process
⇒ ΔSrev = ∫ dQ/T
for an irreversible process, ΔS is not the same as in a reversible process, since more than one reversible process is needed for the two ΔS to be equal.
⇒ ΔSirrev = ΔSrev1 + ΔSrev2 + ....
but if the initial and final states are the same, ΔS for an irreversible process can be calculated as if it were a reversible process.
⇒ ΔSirrev = ΔSrev
Answer:
47.5 mL
Solving:
M1 = 4.00 M
V1 = ?
M2 = 0.760 M
V2 = 0.250 L
---
M1 * V1 = M2 * V2
V1 = ( M2 * V2 ) / M1
V1 = ( 0.760 * 0.250 ) / 4.00
V1 = ( 0.190 ) / 4.00
V1 = 0.0475 L