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Jobisdone [24]
3 years ago
13

A substance is matter that has a definite composition. TRUE or FALSE?

Chemistry
2 answers:
Lina20 [59]3 years ago
6 0

Answer:

FALSE!!

Explanation: some substances like gas or liquid do not have a definite composition/shape

Greeley [361]3 years ago
3 0

Answer: false

Explanation:

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mixer [17]
I don’t know what to answer
6 0
2 years ago
Calculate the percent yield when 500 grams of carbon dioxide react with an excess of water to produce 640 grams of carbonic acid
Elena-2011 [213]

Answer:

Percent yield =  90.5%

Explanation:

Given data:

Mass of carbon dioxide = 500 g

Mass of water = excess

Actual yield of carbonic acid = 640 g

Percent yield = ?

Solution:

Balanced chemical equation:

CO₂ + H₂O  → H₂CO₃

Number of moles of carbon dioxide

Number of moles  = Mass / molar mass

Number of moles = 500 g/ 44 g/mol

Number of moles = 11.4 mol

Now we will compare the moles of H₂CO₃ with CO₂.

                              CO₂          :              H₂CO₃

                                 1             :                  1

                               11.4           :                11.4

Mass of carbonic acid:

Mass = number of moles × molar mass

Mass = 11.4 mol × 62.03 g/mol

Mass = 707.14 g

Percent yield:

Percent yield = actual yield / theoretical yield × 100

Percent yield =  640 g/ 707.14 g × 100

Percent yield =  90.5%

7 0
3 years ago
How many grams of HNO3 are produced when 59.0 g of NO2 completely reacts?
Anettt [7]

Answer:

53.7 grams of HNO3 will be produced

Explanation:

Step 1: Data given

Mass of NO2 = 59.0 grams

Molar mass NO2 = 46.0 g/mol

Step 2: The balanced equation

3NO2 + H2O→ 2HNO3 + NO

Step 3: Calculate moles NO2

Moles NO2 = 59.0 grams / 46.0 g/mol

Moles NO2 = 1.28 moles

Step 4: Calculate moles HNO3

For 3 moles NO2 we need 1 mol H2O to produce 2 moles HNO3 and 1 mol NO

For 1.28 moles NO2 we'll have 2/3 * 1.28 =0.853 moles HNO3

Step 7: Calculate mass HNO3

Mass HNO3 = 0.853 moles * 63.01 g/mol

Mass HNO3 = 53.7 grams

53.7 grams of HNO3 will be produced

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