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KengaRu [80]
3 years ago
5

onsider the reaction, which takes place at a certain elevated temperature CO(g)+NH3(g)⇌HCONH2(g), Kc=0.860 If a reaction vessel

initially contains only CO and NH3 at concentrations of 1.00 M and 2.00 M, respectively, what will the concentration of HCONH2 be at equilibrium?
Chemistry
1 answer:
Zarrin [17]3 years ago
6 0

Answer:

<h2> concentration of HCONH2 at equillibrium is 0.5 M</h2>

Explanation:

                               CO(g) + NH3(g) ⇌ HCONH2(g)

-vessel iniatial             1             2                 0

concentration

-equillibrium              1-x         2-x               x

concentration

                                K_{C} = (CO)\times (NH_{3})/ (HCONH_{2})

                               0.860 = (1-x)(2-x) / x

                                 x^{2}-3.86x+2

                                  x = 3 , 0.5

         concentration of HCONH2 at equillibrium is 0.5 M

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Answer:

No, because Flourine can only form 1 bond, thus backbonding is not obtainable

4 0
2 years ago
What is the pH of a solution with a concentration of 1.8 × 10-4 molar H3O+?
Andre45 [30]
PH is defined as the negative log of Hydrogen ion concentration. Mathematically we can write this as:

pH=-log[H^{+}]=-log[H_{3}O]

We are given the concentration of H_{3}O. Using the value in formula, we get:

pH=-log[1.8*10^{-4}]=3.745

Therefore, the pH of the solution will be 3.745
8 0
3 years ago
5. A sample of benzene (C6H6), weighing 7.05 g underwent combustion in a bomb calorimeter by the following reaction:
Cloud [144]

Answer:

A sample of benzene (C6H6), weighing 7.05 g underwent combustion in a bomb calorimeter by the following reaction:

2 C6H6 (l) + 15 O2 (g) → 12 CO2 (g) + 6 H2O (l)

The heat given off was absorbed by 500 g of water and caused the temperature of the water and the calorimeter to rise from 25.00 to 53.13 oC. The heat capacity of water = 4.18 J/g/oC and the heat capacity of the calorimeter = 10.5 kJ/oC. (1) what is the ΔH of the reaction?

Explanation:

The heat energy released by the reaction = heat absorbed by calorimeter + heat absorbed by water

Heat absorbed by water = mass of water x specific heat capacity of water x change in temperature

Heat absorbed by water =  500 g x 4.18 J/g. oC x (53.13-25.00)oC

                                         = 58791.7 J

Heat absorbed by calorimeter = heat capacity of calorimeter x change in temperature

Heat absorbed by calorimeter = 10.5 x 10^3 J /oC  x (53.13-25.00)oC

                                                  =295365 J

Total heat energy absorbed = 58791.7 J + 295365 J  = 354156.7 J

Number of moles of benzene given is:

number of moles = goven mass of benzene /its molar mass

=7.05 g / 78.0 g/mol

=0.0903mol

Hence, the heat released by the reaction is:

= 354156.7 J / 0.0903 mol

=  3922.00 kJ/mol

Answer:

The heat released during the combustion of 7.05g of benzene is 3922.00kJ/mol.                                              

7 0
2 years ago
URGENT!!! A car engine uses the combustion of fuel to move a system of gears that move its wheels. Not all of the fuel's energy
Jobisdone [24]

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5 0
3 years ago
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17. Which of the following is NOT an empirical formula? *
Aloiza [94]

Answer: 17) d. C_2H_6

18. c. The empirical formula of a compound can be twice the molecular formula.

Explanation:

Molecular formula is the chemical formula which depicts the actual number of atoms of each element present in the compound.  

Empirical formula is the simplest chemical formula which depicts the whole number of atoms of each element present in the compound.  

To calculate the molecular formula, we need to find the valency which is multiplied by each element to get the molecular formula.

The equation used to calculate the valency is:

n=\frac{\text{molecular mass}}{\text{empirical mass}}

The empirical mass can be calculated from empirical formula and molar mass must be known.

17. Thus the empirical formula of C_2H_6 should be CH_3

18. The molecular formula will either be same as empirical formula or is a whole number multiple of empirical formula. Thus the empirical formula of a compound can never be twice the molecular formula.

3 0
3 years ago
Read 2 more answers
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