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Readme [11.4K]
3 years ago
10

How many moles in 3.69 x 10^30 molecules of carbon dioxide?

Chemistry
1 answer:
elixir [45]3 years ago
7 0

Answer:

four million two hundred and thirty

Explanation:

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Pls help! 2CO + O2 → 2CO2
jok3333 [9.3K]

The bond energy of each carbon-oxygen bond in carbon dioxide is d. 736 kJ

Since the chemical reaction is 2CO + O₂ → 2CO₂ and the total bond energy of the products carbon dioxide CO₂ is 1,472 kJ.

Since from the chemical reaction, we have 2 moles of CO₂ which gives 1,472 kJ and there are two carbon-oxygen, C-O bonds in CO₂, then

2 × C-O bond = 1,472 kJ

1 C-O bond = 1.472 kJ/2

C-O bond = 736 kJ

So, the bond energy of each carbon-oxygen bond in carbon dioxide is d. 736 kJ

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7 0
2 years ago
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How many atoms of carbon are in the sample
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There are six atoms in the carbon
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What do the coefficients located before certain molecules in each chemical equation represent?
olga55 [171]
It represents the number of moles required of that molecule to balance the chemical equation, which means to have the reaction chemically happen and goes to completion.

For example:
CH4 + O2 --> H2O + CO2     that is not balanced

with the coefficients located
CH4 + 2O2 --> 2H2O + CO2    now with the coefficients the number of oxygen and hydrogen on each side are equal
6 0
3 years ago
What is the mass of 2.9 moles of calcium? Show all work!
4vir4ik [10]

Answer:

the mass of 2.9 moles of calcium is 116 g

Explanation:

The computation of the mass of 2.9 moles of calcium is shown below

As we know that

Mole = mass ÷  molar mass

where,

Moles be 2.9

And, we know that the molar mass of calcium be 40g/mol

Now put the values to the above formula

2.9 = Mass ÷ 40

So, the mass would be

= 40 × 2.9

=   116 g

Hence, the mass of 2.9 moles of calcium is 116 g

6 0
2 years ago
Never mind jhvjycdtrsesetdfyguhbjnk
OlgaM077 [116]

Complete Question

methanol can be synthesized in the gas phase by the reaction of gas phase carbon monoxide with gas phase hydrogen, a 10.0 L reaction flask contains carbon monoxide gas at 0.461 bar and 22.0 degrees Celsius. 200 mL of hydrogen gas at 7.10 bar and 271 K is introduced. Assuming the reaction goes to completion (100% yield)

what are the partial pressures of each gas at the end of the reaction, once the temperature has returned to 22.0 degrees C express final answer in units of bar

Answer:

The partial  pressure of  methanol is  P_{CH_3OH_{(g)}} =0.077 \  bar

The partial  pressure of carbon monoxide is  P_{CO} = 0.382 \ bar

The partial  pressure at  hydrogen is  P_H =  O \  bar

Explanation:

From the question we are told that

  The volume of the  flask is  V_f = 10.0 \  L

   The initial pressure of carbon monoxide gas is  P_{CO} = 0.461 \ bar

   The initial  temperature of carbon monoxide gas is T_{CO} = 22.0^oC

   The volume of the hydrogen gas is  V_h  =  200 mL = 200 *10^{-3} \  L

    The initial  pressure of the hydrogen is P_H  =  7.10 \  bar

    The initial temperature of the hydrogen  is  T_H = 271 \  K

The reaction of  carbon monoxide and  hydrogen is  represented as

         CO_{(g)} + 2H_2_{(g)} \rightarrow CH_3OH_{(g)}

Generally from the ideal gas equation the initial number of moles of carbon monoxide is  

        n_1  =  \frac{P_{CO} *  V_f }{RT_{CO}}

Here R is the gas constant with value  R  = 0.0821 \ L \cdot atm \cdot mol^{-1} \cdot K

=>     n_1  =  \frac{0.461  *  10 }{0.0821 * (22 + 273)}

=>     n_1  = 0.19

Generally from the ideal gas equation the initial number of moles of Hydrogen  is  

       n_2  =  \frac{P_{H} *  V_H }{RT_{H}}

      n_2  =  \frac{ 7.10 *  0.2 }{0.0821 * 271 }

=> n_2  =  0.064

Generally from the chemical equation of the reaction we see that

        2 moles of hydrogen gas reacts with 1 mole of CO

=>      0.064 moles of  hydrogen gas will react with  x  mole of  CO

So

          x = \frac{0.064}{2}

=>       x = 0.032 \ moles \ of  \  CO

Generally from the chemical equation of the reaction we see that

        2 moles of hydrogen gas reacts with 1 mole of CH_3OH_{(g)}

=>      0.064 moles of  hydrogen gas will react with  z  mole of  CH_3OH_{(g)}

So

          z = \frac{0.064}{2}

=>       z = 0.032 \ moles \ of  \ CH_3OH_{(g)}

From this calculation we see that the limiting reactant is hydrogen

Hence the remaining CO after the reaction is  

          n_k = n_1 - x

=>       n_k = 0.19  - 0.032

=>       n_k = 0.156

So at the end of the reaction , the partial pressure for  CO is mathematically represented as

      P_{CO} = \frac{n_k  *  R *  T_{CO}}{V}

=>    P_{CO} = \frac{0.158   *  0.0821 *  295}{10}

=>    P_{CO} = 0.382 \ bar

Generally the partial pressure of  hydrogen is  0 bar because hydrogen was completely consumed given that it was the limiting reactant

Generally the partial  pressure of the methanol is mathematically represented as

         P_{CH_3OH_{(g)}} = \frac{z  *  R *  T_{CO}}{V_f}

Here  T_{CO} is used because it is given the question that the   temperature  returned to 22.0 degrees C

So

      P_{CH_3OH_{(g)}} = \frac{0.03 * 0.0821 *  295}{10}

     P_{CH_3OH_{(g)}} =0.077 \  bar

6 0
2 years ago
Read 2 more answers
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