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3 years ago

Which statement regarding the Calvin cycle is false?

Chemistry

1 answer:

scoundrel [369]3 years ago

3 0

Answer:

The statement "Six turns of the cycle are required for every glucose molecule later produced in non–Calvin cycle reactions" is incorrect. It really looks not well-worded.

Explanation:

It is incorrect because Six turns of the cycle are required for every glucose molecule produced in Calvin cycle reactions, no in non-Calvin cycle reactions. This process includes the fixation of 6 molecules of carbon dioxide to produce 1 Glucose (seen as the addition of the two Phosphoglyceraldehide molecules (PGAL). Moreover, the other statements in the questions are correct:

ATP is required during carbon fixation.

The most intensive energy phase is reduction and sugar production.

Twelve NADPH are required for every six CO2 fixed.

NADPH is required for reduction and sugar production.

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A 7.0 g sample of a hydrocarbon (a molecule that has only hydrogen and carbon) is subject to combustion analysis. The mass of CO

Akimi4 [234]

Answer: The empirical formula for the given compound is $CH_2$

Explanation:

The chemical equation for the combustion of compound having carbon and hydrogen follows:

$C_xH_y+O_2\rightarrow CO_2+H_2O$

where, 'x' and 'y' are the subscripts of carbon and hydrogen respectively.

We are given:

Mass of $CO_2=22.0g$

We know that:

Molar mass of carbon dioxide = 44 g/mol

For calculating the mass of carbon:

In 44 g of carbon dioxide, 12 g of carbon is contained.

So, in 22.0 g of carbon dioxide, $\frac{12}{44}\times 22.0=6g$ of carbon will be contained.

For calculating the mass of hydrogen:

Mass of hydrogen = Mass of sample - Mass of carbon

Mass of hydrogen = 7.0 g - 6 g

Mass of hydrogen = 1.0 g

To formulate the empirical formula, we need to follow some steps:

Step 1: Converting the given masses into moles.

Moles of Carbon = $\frac{\text{Given mass of Carbon}}{\text{Molar mass of Carbon}}=\frac{6g}{12g/mole}=0.5moles$

Moles of Hydrogen = $\frac{\text{Given mass of Hydrogen}}{\text{Molar mass of Hydrogen}}=\frac{1.0g}{1g/mole}=1.0moles$

Step 2: Calculating the mole ratio of the given elements.

For the mole ratio, we divide each value of the moles by the smallest number of moles calculated which is 0.5 moles.

For Carbon = $\frac{0.5}{0.5}=1$

For Hydrogen = $\frac{1.0}{0.5}=2$

Step 3: Taking the mole ratio as their subscripts.

The ratio of Fe : C : H = 1 : 2

Hence, the empirical formula for the given compound is $C_{1}H_{2}=CH_2$

4 0

3 years ago

Why is making a peanut pretzel and cereal mixture

guajiro [1.7K]

It is two or more objects and different things that can be removed from each other.

7 0

2 years ago

If a compound has a molar más of 180g/mol and it’s empirical formula is CH^2O, what is it’s molecular formula?

lesya [120]

C: 12.0107 g/mol ≅ 12.00 g/mol

H: 1.00784 g/mol ≅ 1.008 g/mol

O: 15.999 g/mol ≅ 16.00 g/mol

n(molar mass of CH2O)= 180

n.30=180

n=6

molecular formula: c6h12o6 glucose

4 0

2 years ago

How much smaller is an electron than a proton

meriva

Answer:

An electron is around 1800 times smaller than a proton

Explanation:

3 0

3 years ago

Read 2 more answers

Calcium chloride has a melting point of 772°C, and water has a boiling point of 100°C. Which statement is true for calcium chlor

nekit [7.7K]

The difference is due to the fact that calcium chloride has stronger intermolecular forces than water.

4 0

3 years ago