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3 years ago

When using the benedict's assay, which color would indicate the most reducing sugar present?

1 answer:

3 0

Brick-red because the most reducing sugar reduces the blue copper salts -that are present in Benedict's solution- to a red compound.

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Compound A is an organic compound which contains Carbon, Hydrogen and Oxygen. When 0.240g of the vapour of A is slowly passed ov

vesna_86 [32]

(a) In this section, give your answers to three decimal places.

(i)

Calculate the mass of carbon present in 0.352 g of CO

Use this value to calculate the amount, in moles, of carbon atoms present in 0.240 g

(ii)

Calculate the mass of hydrogen present in 0.144 g of H

Use this value to calculate the amount, in moles, of hydrogen atoms present in 0.240 g

(iii)

Use your answers to calculate the mass of oxygen present in 0.240 g of

Use this value to calculate the amount, in moles, of oxygen atoms present in 0.240 g

(b)

Use your answers to

(a)

to calculate the empirical formula of

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4 0

3 years ago

What principle chemistry

NNADVOKAT [17]

Is this a question ?

8 0

3 years ago

Identify the oxidizing agent and the reducing agent for 4Li(s) + O_2 (g) to 2Li_2O(s).

Doss [256]

The reaction is:

<span>4Li(s) + O2 (g) = 2Li+ + 2O-2(s).

The oxidizing agent is the one that is being reduced which is oxygen where the charge changed from neutral to -2 while the reducing agent is the on being oxidized which is lithium where the charge change from neutral to +1.</span>

7 0

3 years ago

Which of these pairs of elements is most likely to be part of a polyatomic ion?

Mrrafil [7]

S and O would be on a polyatomic ion as I know of

3 0

3 years ago

Read 2 more answers

What effect does a) increasing the total pressure and b) increasing the temperature have on the equilibrium H2(g) CO2(g) D H2O(g

Rama09 [41]

Answer:

d. a) no change in the equilibrium and

b) equilibrium shifts towards products.

Explanation:

Hello.

In this case, for the reaction:

$H_2(g) +CO_2(g) \rightleftharpoons H_2O(g)+ CO(g);\ \ \ \ \Delta H=41.2kJ/mol$

Which is endothermic due to the positive enthalpy of reaction. In such a way, based on the Le Chatelier's principle which states that increasing the temperature of an endothermic chemical reaction shifts the equilibrium towards products as heat is understood as a reactant, we can see, this is the case.

Moreover, since the change in the number of gaseous moles in the chemical reaction (coefficients balancing the reaction) is 0 (1+1-1-1), we can see that increasing the total pressure does not have any effect over equilibrium.

Therefore answer is d. a) no change in the equilibrium and b) equilibrium shifts towards products.

Best regards!

6 0

2 years ago