Answer:
D)both the forward and reverse reactions continue.
Explanation:
Chemical equilibrium can be regarded as state whereby rate of the forward reaction is equal to rate of backward reaction. It should be noted that At equilibrium both the forward and reverse reactions continue.
Answer:
Option A. 1.14L
Explanation:
Data obtained from the question include:
V1 = 1.20 L
P1 = at stp = 760torr
T1 = at stp = 273K
P2 = 900torr
T2 = 35°C = 35 + 273 = 308K
V2 =?
Using P1V1/T1 = P2V2/T2, we can obtain the new volume as follows:
P1V1/T1 = P2V2/T2
(760 x 1.2)/273 = (900 x V2) /308
Cross multiply to express in linear form
273 x 900 x V2 = 760 x 1.2 x 308
Divide both side by 273 x 900
V2 = (760 x 1.2 x 308) /(273 x 900)
V2 = 1.14L
Answer:
14.29g
Explanation:
First, let us write a balanced equation for the reaction. This is illustrated below below:
4Fe + 3O2 —> 2Fe2O3
Next, let us calculate the mass of Fe that reacted and the mass of Fe2O3 produced from the balanced equation. This is shown below:
Molar Mass of Fe = 56g/mol
Mass of Fe from the balanced equation = 4 x 56 = 224g
Molar Mass of Fe2O3 = (56x2) + (16x3) = 112 + 48 = 160g/mol
Mass of Fe2O3 from the balanced equation = 2 x 160 = 320g
From the balanced equation,
224g of Fe produced 320g of Fe2O3.
Therefore, 10g of Fe will produce = (10x320)/224 = 14.29g of Fe2O3
From the calculations made above, 10g iron(Fe) produced 14.29g of iron(iii) oxide (Fe2O3)
