Ask question

Ask question

All categories

3 years ago

14

. How many grams of water would require 4400 joules

1 answer:

Alja [10]3 years ago

5 0

Answer:

The specific heat of water is 4.18 J/g C.

Explanation:

q

=

m

C

s

Δ

T

Never forget that!

2200

=

m

⋅

4.18

J

g

⋅

°

C

⋅

66

°

C

∴

m

≈

8.0

g

You might be interested in

BRAINLIEST IF CORRECT

Airida [17]

Answer:

When water vapor in the air comes into contact with something cool, its molecules slow down and get closer together.

Explanation:

I hate it when you accidently drop your drink haha. Have a good day!!

3 0

3 years ago

Read 2 more answers

Magnesium reacts with hydrochloric acid, HCl, to form magnesium chloride and hydrogen gas. The reaction is: Mg + 2HCl → MgCl2 +

prisoha [69]

Answer is: mass of HCl is 15,6 g.
Chemical reaction: Mg + 2HCl → MgCl₂ + H₂.
m(Mg) = 5,2 g.
n(Mg) = m(Mg) ÷ M(Mg).
n(Mg) = 5,2 g ÷ 24,3 g/mol.
n(Mg) = 0,213 mol.
From chemical reaction: n(Mg) : n(HCl) = 1 : 2.
n(HCl) = 0,426 mol.
m(HCl) = 0,426 mol · 36,45 g/mol.
m(HCl) = 15,6 g.

5 0

3 years ago

[H3O+] = 3.6 x 10-2 M

spayn [35]

Answer:

Explanation:

Hello there!

In this case, since this concentration of hydronium ions is given, we infer we may calculate that of the hydroxide ions, pH and pOH because no question was specifically given. That is why we proceed as follows:

- pH: Here, we use this concentration to calculate the pH according to the negative logarithm:

$pH=-log(3.6x10^{-2})=1.44$

Which means that the solution is acidic as the pH is less than 7.

- pOH: since the pH added to the pOH is 14, we can calculate the latter as follows:

$pOH=14-1.44=12.56$

- Hydroxide concentration: Given the pOH, we apply the antilogarithm to calculate such concentration as shown below:

$[OH^-]=10^{-pOH}=10^{12.56}=2.75x10^{-13}M$

Keep in mind, this is an arbitrary solution because no question was provided.

Regards!

7 0

3 years ago

Given the lattice energy of NaBr = 736 kJ/mol, the ionization energy of Na = 496 kJ/mol and the electron affinity of Br = −325 k

mars1129 [50]

Answer : The value of $\Delta H^o$ for the reaction is, -565 kJ/mol

Explanation :

The formation of sodium bromide is,

$Na(g)+Br(g)\overset{\Delta H^o}\rightarrow NaBr(s)$

$\Delta H^o$ = enthalpy of the reaction

The steps involved in the reaction are:

(1) Conversion of gaseous sodium atoms into gaseous sodium ions.

$Na(g)\overset{\Delta H_I}\rightarrow Na^{+1}(g)$

$\Delta H_I$ = ionization energy of sodium = 496 kJ/mol

(2) Conversion of gaseous bromine atoms into gaseous bromine ions.

$Br(g)\overset{\Delta H_E}\rightarrow Br^-(g)$

$\Delta H_E$ = electron affinity energy of bromine = -325 kJ/mol

(3) Conversion of gaseous cations and gaseous anion into solid sodium bromide.

$Na^+(g)+Br^-(g)\overset{\Delta H_L}\rightarrow NaBr(s)$

$\Delta H_L$ = lattice energy of sodium bromide = -736 kJ/mol

To calculate the $\Delta H^o$ for the reaction, the equation used will be:

$\Delta H^o=\Delta H_I+\Delta H_E+\Delta H_L$

Now put all the given values in this equation, we get:

$\Delta H^o=496kJ/mole+(-325kJ/mole)+(-736kJ/mole)$

$\Delta H^o=-565kJ/mole$

Therefore, the value of $\Delta H^o$ for the reaction is, -565 kJ/mol

7 0

3 years ago

In the following reaction, how many liters of oxygen will react with 124.5 liters of propane (C3H8), at STP?

nexus9112 [7]

In the following reaction,76.616 litre of oxygen will react

8 0

3 years ago