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Elena-2011 [213]

3 years ago

7

I WILL RATE BRAINLIEST!!!

1 answer:

Naddik [55]3 years ago

4 0

<span>the answer:
The net ionic equation,
H3PO4 (aq) + 3 OH− (aq)------- PO4−3 (aq) + 3 H2O (l),

</span> H3PO4 is a strong acid, (presence of hydrogen H)
OH- is a strong base, (presence of OH-)

so the true answer is <span>strong acid-strong base</span>

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What is the difference between chemical and physical change with respect

kozerog [31]

Answer:

Physical changes are changes that do not alter the identity of a substance. Chemical changes are changes that occur when one substance is turned into another substance.

Explanation:

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When this reaction in equilibrium is heated, a red/brown color persists. what is true about this reaction? 2no2(

dimulka [17.4K]

NO₂ is a brown gas while N₂O₄ is colorless. If heating causes a brown color to persist, then this means that heating causes the reaction to shift backwards and produce NO₂. Therefore, the reaction must be exothermic.

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3 years ago

What is the percent of hydrogen peroxide in the solution when 5.02g of H2O2 solution reacts to produce 0.153g of H2O2? 2H2O2 (l)

Murljashka [212]

<u>Given:</u>

Mass of H2O2 solution = 5.02 g

Mass of H2O2 = 0.153 g

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The % H2O2 in solution

<u>Explanation:</u>

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5 0

3 years ago

5 moles of an ideal gas (Cp = 3R, Cv 2R ) are heated from 25°C to 300°C. Calculate (a) The change in internal energy of the gas

Artist 52 [7]

Answer :

(a) The change in internal energy of the gas is 22.86 kJ.

(b) The change in enthalpy of the gas is 34.29 kJ.

Explanation :

(a) The formula used for change in internal energy of the gas is:

$\Delta U=nC_v\Delta T\\\\\Delta U=nC_v(T_2-T_1)$

where,

$\Delta U$ = change in internal energy = ?

n = number of moles of gas = 5 moles

$C_v$ = heat capacity at constant volume = 2R

R = gas constant = 8.314 J/mole.K

$T_1$ = initial temperature = $25^oC=273+25=298K$

$T_2$ = final temperature = $300^oC=273+300=573K$

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

$\Delta U=nC_v(T_2-T_1)$

$\Delta U=(5moles)\times (2R)\times (573-298)$

$\Delta U=(5moles)\times 2(8.314J/mole.K)\times (573-298)$

$\Delta U=22863.5J=22.86kJ$

The change in internal energy of the gas is 22.86 kJ.

(b) The formula used for change in enthalpy of the gas is:

$\Delta H=nC_p\Delta T\\\\\Delta H=nC_p(T_2-T_1)$

where,

$\Delta H$ = change in enthalpy = ?

n = number of moles of gas = 5 moles

$C_p$ = heat capacity at constant pressure = 3R

R = gas constant = 8.314 J/mole.K

$T_1$ = initial temperature = $25^oC=273+25=298K$

$T_2$ = final temperature = $300^oC=273+300=573K$

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

$\Delta H=nC_p(T_2-T_1)$

$\Delta H=(5moles)\times (3R)\times (573-298)$

$\Delta H=(5moles)\times 3(8.314J/mole.K)\times (573-298)$

$\Delta H=34295.25J=34.29kJ$

The change in enthalpy of the gas is 34.29 kJ.

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3 years ago