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blondinia [14]
2 years ago
8

Determine the direction that each of the reactions will progress. Assume that the reactants and products are present in equimola

r amounts. The standard free energy of hydrolysis of ATP is – 30.5 kJ / mol.
Chemistry
1 answer:
xxMikexx [17]2 years ago
8 0

Answer:

It would move either left or right

Explanation: Taking assumption that,

Fructose + ATP fructose - 6 - phosphate + ADP (The standard free energy of hydrolysis for fructose-6-phosphate is - 15.9 kJ/mol.) 3 - phosphoglycerate + ATP 1,3 - bisphosphoglycerate + ADP (The standard free energy of hydrolysis for 1,3-bisphosphoglycerate is - 4 9.3 kJ/mol.) pyruvate + ATP phosphoenolpyruvate + ADP (The standard free energy of hydrolysis for phosphoenolpyruvate -is -61.9 kJ/mol.)

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Which statement accurately describes liquids?
Zielflug [23.3K]
C. they expand to fill all the space
3 0
3 years ago
5. Which contains more nitrogen: 60g of urea, (NH2)2CO, or 100g of ammonium sulphate, (NH4)2SO4
topjm [15]

Answer:

Urea contains more nitrogen

Explanation:

1 mole of Urea contains 2 moles of Nitrogen and 1 mole of ammonium sulfate contains, also, 2 moles of nitrogen.

60g of urea (Molar mass: 60g/mol) contains:

60g × (1mol / 60g) = 1 mole. As 1 mole of urea contains 2 moles of nitrogen, moles of nitrogen are 2.

100g of ammonium sulfate (Molar mass: 132g/mol) contains:

100g × (1mol / 132g) = 0.758 moles.

As 1 mole of urea contains 2 moles of nitrogen, moles of nitrogen are 0.758×2 = 1.516 moles.

That means, <em>urea contains more nitrogen</em>.

5 0
3 years ago
Please hurry asap I WILL MARK BRAINLEST
gulaghasi [49]

Answer:

an endothermic reaction

Explanation:

An endothermic reaction has occurred.

4 0
3 years ago
Read 2 more answers
Suppose 2.4 g of Mg reacts with 10.0 g of O2, to create magnesium oxide. How much magnesium oxide is produced?
o-na [289]

Answer:

3.98 g

Explanation:

Step 1. Write the balanced chemical reaction. In this case, magnesium reacts with oxygen to produce magnesium oxide:

2~Mg(s) + O_2 (g)\rightarrow 2~MgO (s)

\\

Step 2. Calculate the number of moles of magnesium:

n_{Mg} = \frac{2.4~g}{24.305~g/mol} = 0.0987~mol

\\

Step 3. Calculate the number of moles of oxygen:

n_{O_2} = \frac{10.0~g}{32.00~g/mol} = 0.3125~mol

\\

Step 4. Identify the limiting reactant comparing the equivalents. Equivalent of Mg:

eq_{Mg} = \frac{0.0987~mol}{1} = 0.0987~mol

Equivalent of oxygen:

eq_{O_2} = \frac{0.3125~mol}{2} = 0.15625~mol

Therefore, Mg is the limiting reactant.

\\

Step 5. According to the stoichiometry of this reaction:

n_{Mg} = n_{MgO} = 0.0987~mol

\\

Step 6. Convert the number of moles of MgO into mass:

m_{MgO} = 0.0987~mol\cdot 40.304~g/mol = 3.98~g

5 0
3 years ago
Gaseous methane will react with gaseous oxygen to produce gaseous carbon dioxide and gaseous water . Suppose 9.3 g of methane is
Marrrta [24]

Answer:

26 g

Explanation:

Write the balanced reaction first

CH4 + 2 O2 --> CO2 + 2 H2O

9.3g + 52.3g --> ? CO2

You must determine how much carbon dioxide can be made from each of the reactants. The maximum mass that can be made is the lower of the two.

From CH4:

9.3g CH4 (1molCH4/16.05gCH4) (1molCO2 / 1molCH4) (44.01g CH4 / 1molCO2) = 26 g

From O2:

52.3g O2 (1molO2/32gO2) (1molCO2/2molO2)(44.01g/1molCO2) = 36 g

6 0
3 years ago
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