A combustion reaction involves an organic compound reacted with oxygen. The general chemical equation is as follows:
<span>
Organic Compound + Oxygen = CO2 + H2O
</span><span>To calculate the amount of C present in the original sample, we use the values given and assume that there is complete combustion that is happening.
</span><span>
7.33 g CO2 ( 1 mol CO2 / 44.01 g CO2)(1 mol C / 1 mol CO2) = 0.167 mol C
Therefore, 0.167 mol of C was originally in the sample.</span>
Answer:
45 °C.
Explanation:
From the question given above, the following data were obtained:
Heat (Q) = 1125 J
Mass (M) = 250 g
Final temperature (T₂) = 55 °C
Specific heat capacity (C) = 0.45 J/gºC
Initial temperature (T₁) =?
The initial temperature of the iron can be obtained as illustrated below:
Q = MC(T₂ – T₁)
1125 = 250 × 0.45 (55 – T₁)
1125 = 112.5 (55 – T₁)
Divide both side by 112.5
1125/112.5 = 55 – T₁
10 = 55 – T₁
Collect like terms
10 – 55 = –T₁
–45 = –T₁
Multiply through by –1
45 = T₁
T₁ = 45 °C
Therefore, the initial temperature of the iron is 45 °C
I think it is b.heat transfers to his body from the water by conduction
Answer:
Explanation:
To find the theoretical yield of the equation. First identify the limiting reactant in a chemical equation.
Step 1: write out the equation and balance it.
Al+ 3mno2=3mn+ 2Alo3.
The limiting reactant is mn02 because it is not found in excess.
Step 2: convert the % to gram . All contain 67.2% mole and mno2 will be 100-67.2= 32.8
All=67.2÷100×290(total gram of the reactants)=194.88g
Mno2=32.8÷100×290g=94.12g.
Step 3:calculate the molar mass of mno2 and that of mn. The atomic mass of mn is 54.9380 and that of oxygen is 16.
Mno2=54.938+ (16)2=86.98g/mol.
Mn=54.938.
Step 4:
From your balanced equation , calculate mn.
94.12g mno2× (1mol mno2÷86.98(molarmass) of mno2×3 mol of mn/4molAl×54.938g of mn÷1mol of mn.
94.12g×1÷86.98g×3÷4×54.938÷1
=44.58g
Answer:
- <em><u>Option a. no change</u></em>
Explanation:
The question makes sense only if the equation is an equilibrium reaction:
- <em>4A (g) + 5B (g) ⇄ 2C (g) + 7D (g) </em>
This is, A and B react to produce C and D, forward reaction; and C and D react to form A and B, reverse reaction.
Then, you can study the effect of increased pressure using LeChatelier's principle.
To counteract the disturbing effect produced by increased pressure on the equilibrium, the system will react shifting the toward to the side where the pressure could be decreased.
That would be toward the side that has less gas molecules.
Since both sides have 9 molecules (4 + 5 = 2 + 7 = 9), the equilibrium concetrations will not change.
That is represented by the first choice: no change.
