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2 years ago

8

If you subtract an objects starting velocity from its final velocity and divide by the time it took to change velocity, what are

you finding

1 answer:

amid [387]2 years ago

7 0

Change in velocity over time is acceleration.

You're finding acceleration .

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In order to become ________, ions will combine with other ions to form new substances.

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A 20.0-g sample of sugar is dissolved in 59.8 g of water. What is the concentration of the solution?

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2 years ago

A critical reaction in the production of energy to do work or drive chemical reactions in biological systems is the hydrolysis o

MAVERICK [17]

Answer : The value of $\Delta G_{rxn}$ is -49.6 kJ/mol

Explanation :

First we have to calculate the reaction quotient.

Reaction quotient (Q) : It is defined as the measurement of the relative amounts of products and reactants present during a reaction at a particular time.

The given balanced chemical reaction is,

$ATP(aq)+H_2O(l)\rightarrow ADP(aq)+HPO_4^{2-}(aq)$

The expression for reaction quotient will be :

$Q=\frac{[ADP][HPO_4^{2-}]}{[ATP]}$

In this expression, only gaseous or aqueous states are includes and pure liquid or solid states are omitted.

Given:

$[ATP]$ = 5.0 mM

$[ADP]$ = 0.60 mM

$[HPO_4^{2-}]$ = 5.0 mM

Now put all the given values in this expression, we get

$Q=\frac{(0.60)\times (5.0)}{(5.0)}=0.60mM=0.60\times 10^{-3}M$

Now we have to calculate the value of $\Delta G_{rxn}$ .

The formula used for $\Delta G_{rxn}$ is:

$\Delta G_{rxn}=\Delta G^o+RT\ln Q$ ............(1)

where,

$\Delta G_{rxn}$ = Gibbs free energy for the reaction = ?

$\Delta G_^o$ = standard Gibbs free energy = -30.5 kJ/mol

R = gas constant = $8.314\times 10^{-3}kJ/mole.K$

T = temperature = $37.0^oC=273+37.0=310K$

Q = reaction quotient = $0.60\times 10^{-3}$

Now put all the given values in the above formula 1, we get:

$\Delta G_{rxn}=(-30.5kJ/mol)+[(8.314\times 10^{-3}kJ/mole.K)\times (310K)\times \ln (0.60\times 10^{-3})$

$\Delta G_{rxn}=-49.6kJ/mol$

Therefore, the value of $\Delta G_{rxn}$ is -49.6 kJ/mol

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2 years ago