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Olegator [25]
3 years ago
15

How many grams of CO are needed to react with an excess of Fe2O3 to produce (210.3 g Fe) 209.7 g Fe? Show your work.

Chemistry
2 answers:
Flura [38]3 years ago
6 0
The balanced chemical reaction is given as:

<span>3CO (g) + Fe2O3 (s) --> 2Fe (s) + 3CO2 (g)

We are given the amount of the product to be produced from the reaction. We use this as the starting value for the calculations. We do as follows:

209.7 g Fe ( 1 mol / 210.3 g Fe ) ( 3 mol CO / 2 mol Fe ) (28.01 g / 1 mol) = 41.90 g CO needed</span>
Fed [463]3 years ago
4 0

Explanation:

3CO(g)+Fe_2O_3(s)\rightarrow 2Fe(s)+3CO_2(g)

1)Mass of CO when 210.3 g of Fe produced.

Number of moles of Fe in 210.3 g=

\frac{\text{Given mass of Fe}}{\text{Molar mass of Fe}}

=\frac{210.3}{55.84 g/mol}=3.76 mol

According to reaction, 2 moles of Fe are obtained from 3 moles of CO, then 3.76 moles of Fe will be obtained from : \frac{3}{2}\times 3.76 moles of CO that is 5.64 moles.

Mass of CO in 5.64 moles =

\text{Number of moles}\times \text{molar mass of CO}=5.46\times 28 g/mol=157.92 g

2)Mass of CO when 209.7 g of Fe produced.

Number of moles of Fe in 209.7 g=

\frac{\text{Given mass of Fe}}{\text{Molar mass of Fe}}

=\frac{209.7}{55.84 g/mol}=3.75 mol

According to reaction, 2 moles of Fe are obtained from 3 moles of CO, then 3.75 moles of Fe will be obtained from : \frac{3}{2}\times 3.75 moles of CO that is 5.625 moles.

Mass of CO in 5.625 moles =

\text{Number of moles}\times \text{molar mass of CO}=5.625\times 28 g/mol=157.5 g

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Answer:

I would say, what helps me is really paying attention in class and asking questions, also making sure you study for upcoming test's and quizzes and completely assingments on time

Explanation:

3 0
3 years ago
A weather balloon is filled with helium that occupies a volume of 5.57 104 L at 0.995 atm and 32.0°C. After it is released, it r
Alchen [17]

6.52 × 10⁴ L. (3 sig. fig.)

<h3>Explanation</h3>

Helium is a noble gas. The interaction between two helium molecules is rather weak, which makes the gas rather "ideal."

Consider the ideal gas law:

P\cdot V = n\cdot R\cdot T,

where

  • P is the pressure of the gas,
  • V is the volume of the gas,
  • n is the number of gas particles in the gas,
  • R is the ideal gas constant, and
  • T is the absolute temperature of the gas in degrees Kelvins.

The question is asking for the final volume V of the gas. Rearrange the ideal gas equation for volume:

V = \dfrac{n \cdot R \cdot T}{P}.

Both the temperature of the gas, T, and the pressure on the gas changed in this process. To find the new volume of the gas, change one variable at a time.

Start with the absolute temperature of the gas:

  • T_0 = (32.0 + 273.15) \;\text{K} = 305.15\;\text{K},
  • T_1 = (-14.5 + 273.15) \;\text{K} = 258.65\;\text{K}.

The volume of the gas is proportional to its temperature if both n and P stay constant.

  • n won't change unless the balloon leaks, and
  • consider P to be constant, for calculations that include T.

V_1 = V_0 \cdot \dfrac{T_1}{T_2} = 5.57\times 10^{4}\;\text{L}\times \dfrac{258.65\;\textbf{K}}{305.15\;\textbf{K}} = 4.72122\times 10^{4}\;\text{L}.

Now, keep the temperature at T_1 =258.65\;\text{K} and change the pressure on the gas:

  • P_1 = 0.995\;\text{atm},
  • P_2 = 0.720\;\text{atm}.

The volume of the gas is proportional to the reciprocal of its absolute temperature \dfrac{1}{T} if both n and T stays constant. In other words,

V_2 = V_1 \cdot\dfrac{\dfrac{1}{P_2}}{\dfrac{1}{P_1}} = V_1\cdot\dfrac{P_1}{P_2} = 4.72122\times 10^{4}\;\text{L}\times\dfrac{0.995\;\text{atm}}{0.720\;\text{atm}}=6.52\times 10^{4}\;\text{L}

(3 sig. fig. as in the question.).

See if you get the same result if you hold T constant, change P, and then move on to change T.

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nata0808 [166]

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H2O2 --> H2O + (1/2)O2
This has an equivalent number of H and O atoms on either side, but we want the coefficients to be whole numbers, so we multiply everything by 2:
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The reaction is endothermic as energy is absorbed to break a bond.
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