What is the Protons?

A piece of iron (CsFe = 0.45 J/g·⁰C) with a mass of 4.45 g at temperature of 101.0 oC is dropped into an insulated calorimeter c

OleMash [197]

Answer:

22.75 ⁰C.

Explanation:

The amount of heat added to a substance (Q) can be calculated from the relation:

Q = m.c.ΔT.

where, Q is the amount of heat added,

m is the mass of the substance,

c is the specific heat of the substance,

ΔT is the temperature difference (final T - initial T).

∵ The amount of heat released by Fe = the amount of heat absorbed by water

<em>∴ - (m.c.ΔT) released by Fe = (m.c.ΔT) absorbed by water.</em>

- (4.45 g)(0.45 J/g·⁰C)(final T - 101.0 ⁰C) = (50.0 g)(4.186 J/g·⁰C)(final T - 22.0 ⁰C)

- 2.0025 final T + 202.2525 = 209.3 final T - 4604.

209.3 final T + 2.0025 final T = 202.2525 + 4604

211.3025 final T = 4806.2525.

<em>final T = 4806.2525/211.3025 = 22.75 ⁰C.</em>

3 0

4 years ago

The current human population is reaching nearly eight billion people and will continue to grow. Which are the consequences of po

S_A_V [24]

The population will continue to grow but as we grow so does pollution. Some would need vaccines to cure simple diseases like the flu but what if there would not be enough?

8 0

3 years ago

Read 2 more answers

Determine which of the following statement is correct when the equilibrium constant K for a certain reaction is 10 at 298 K and

aev [14]

Answer:

4. The reaction is spontaneous at any temperatures if the standard entropy of reaction is positive.

Explanation:

Equilibrium constant decreases on increasing the temperature . So the reaction appears to be exothermic . In other words

ΔH is negative .

Δ G = ΔH - TΔS

If ΔS is positive , second term is negative . ΔH is negative so the RHS of the equation is negative at all temperatures . Hence Δ G of the reaction is negative . So reaction is spontaneous at any temperature.

3 0

3 years ago

A reaction A(aq)+B(aq)↽−−⇀C(aq) has a standard free‑energy change of −4.20 kJ/mol at 25 °C. What are the concentrations of A, B,

Dafna1 [17]

Answer : The concentration of $A,B\text{ and }C$ at equilibrium are 0.132 M, 0.232 M and 0.168 M respectively.

Explanation :

The given chemical reaction is,

$A(aq)+B(aq)\rightleftharpoons C(aq)$

First we have to calculate the equilibrium constant for the reaction.

The relation between the equilibrium constant and standard free‑energy is:

$\Delta G^o=-RT \ln k$

where,

$\Delta G^o$ = standard free‑energy change = -4.20 kJ/mole

R = universal gas constant = 8.314 J/mole.K

k = equilibrium constant = ?

T = temperature = $25^oC=273+25=298K$

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

$-4.20kJ/mole=-(8.314J/mole.K)\times (298K) \ln k$

$k=5.45$

Now we have to calculate the concentrations of A, B, and C at equilibrium.

The given equilibrium reaction is,

$A(aq)+B(aq)\rightleftharpoons C(aq)$

Initially 0.30 0.40 0

At equilibrium (0.30-x) (0.40-x) x

The expression of equilibrium constant will be,

$k=\frac{[C]}{[A][B]}$

$5.45=\frac{x}{(0.30-x)\times (0.40-x)}$

By solving the term x, we get

$x=0.168\text{ and }0.716$

From the values of 'x' we conclude that, x = 0.716 can not more than initial concentration. So, the value of 'x' which is equal to 0.716 is not consider.

The value of x will be, 0.168 M

The concentration of $A$ at equilibrium = (0.30-x) = 0.30 - 0.168 = 0.132 M