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BlackZzzverrR [31]
4 years ago
6

Balancing H2SO4+NH4OH —> H2O+(NH4)2SO4

Chemistry
1 answer:
azamat4 years ago
3 0

H₂SO₄   +    2NH₄OH    →     (NH₄)₂SO₄   +    2H₂O

Explanation:

  Unbalanced reaction equation:

                    H₂SO₄   +    NH₄OH    →     (NH₄)₂SO₄   +    H₂O

We can use a simple mathematical approach to balance this equation by solving simple algebraic equations.

         aH₂SO₄   +    bNH₄OH    →     c(NH₄)₂SO₄   +    dH₂O

a,b,c and d are simple coefficients that will balance the equation:

   Conservation of H: 2a + 5b = 8c + 2d

                               S:   a = c

                               O:  4a + b = 4c + d

                               N:   b = 2c

lets assume that a = 1

                             c= 1

                             b = 2

                  Solving for d from 4a + b = 4c + d

                   d = 4a + b -4c = 4(1) + 2 - 4(1) = 2        

 

                  H₂SO₄   +    2NH₄OH    →     (NH₄)₂SO₄   +    2H₂O

Learn more:

Balancing of equations brainly.com/question/6078553

#learnwithBrainly

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How much nitrogen-13 would be left after 40 minutes if the sample started at 4g
BlackZzzverrR [31]
<h3>Answer:</h3>

0.248 g

<h3>Explanation:</h3>

<u>We are given;</u>

  • Time as 40 minutes
  • Original amount of N-13

We are required to calculate the amount left after decay.

  • We need to know the half life of N-13 first;
  • Half life of N-13 is 9 minutes 58 seconds (9.965 minutes0

We are going to use the formula;

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That is; N = N₀ ×  0.5^n , where n is the number of half lives.

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3 0
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A gaseous compound composed of sulfur and oxygen has a density of 9.88 g/L at stp. What is the molar mass of this gas?
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Answer: The molar mass of this gas is 221 g/mol

Explanation:

The relation between density and molar mass is :

PM=dRT

where P = pressure of gas = 1 atm (at STP)

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d = density of gas = ?

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T= temperature of gas = 273 K ( at STP)

1atm\times M=9.88g/L\times 0.0821Latm/Kmol\times 273K

M=221g/mol

Thus the molar mass of this gas is 221 g/mol

6 0
4 years ago
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