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3 years ago

How is salt water classified?

Chemistry

1 answer:

docker41 [41]3 years ago

4 0

Salt water is considered a compound since water is H20 (conpound) and Salt with is NaCl.

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How many grams in 6.20 x 10^25 atoms of bromine (Br) ? image attached , will give brainliest

Deffense [45]

Answer:

8239.2g

Explanation:

Given parameters:

Number of atoms in Br = 6.2 x 10²⁵atoms

Unknown:

Mass of Br = ?

Solution:

From mole concepts, we know that:

1 mole of a substance contains 6.02 x 10²³ atoms/mol

Molar mass of Br = 80g/mol

6.2 x 10²⁵atoms x $\frac{1}{6.02 x 10^{23} }$ $\frac{mol}{atoms}$ x 80 x $\frac{g}{moles}$

= 8239.2g

8 0

3 years ago

*GIVING BRAINLIEST* NEED ANSWER ASAPPP

poizon [28]

Same Question here answered by me with explanation check the link below for your answer.

brainly.com/question/24944271?

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3 years ago

What is meant by collision theory?

Tcecarenko [31]

Answer:

The collision theory states that a chemical reaction can only occur between particles when they collide (hit each other).

hope it helps~

4 0

2 years ago

Which body system is this? Your brain and nerves receive and send

KiRa [710]

Answer: its the nervous system

Explanation:

8 0

3 years ago

Calculate the standard reaction Gibbs free energy for the following cell reactions: (a) 2 Ce41(aq) 1 3 I2(aq) S 2 Ce31(aq) 1 I32

Law Incorporation [45]

Answer:

For a: The standard Gibbs free energy of the reaction is -347.4 kJ

For b: The standard Gibbs free energy of the reaction is 746.91 kJ

Explanation:

Relationship between standard Gibbs free energy and standard electrode potential follows:

$\Delta G^o=-nFE^o_{cell}$ ............(1)

For a:

The given chemical equation follows:

$2Ce^{4+}(aq.)+3I^{-}(aq.)\rightarrow 2Ce^{3+}(aq.)+I_3^-(aq.)$

Oxidation half reaction: $Ce^{4+}(aq.)\rightarrow Ce^{3+}(aq.)+e^-$ ( × 2)

Reduction half reaction: $3I^_(aq.)+2e^-\rightarrow I_3^-(aq.)$

We are given:

$n=2\\E^o_{cell}=+1.08V\\F=96500$

Putting values in equation 1, we get:

$\Delta G^o=-2\times 96500\times (+1.80)=-347,400J=-347.4kJ$

Hence, the standard Gibbs free energy of the reaction is -347.4 kJ

For b:

The given chemical equation follows:

$6Fe^{3+}(aq.)+2Cr^{3+}+7H_2O(l)(aq.)\rightarrow 6Fe^{2+}(aq.)+Cr_2O_7^{2-}(aq.)+14H^+(aq.)$

Oxidation half reaction: $Fe^{3+}(aq.)\rightarrow Fe^{2+}(aq.)+e^-$ ( × 6)

Reduction half reaction: $2Cr^{2+}(aq.)+7H_2O(l)+6e^-\rightarrow Cr_2O_7^{2-}(aq.)+14H^+(aq.)$

We are given:

$n=6\\E^o_{cell}=-1.29V\\F=96500$

Putting values in equation 1, we get:

$\Delta G^o=-6\times 96500\times (-1.29)=746,910J=746.91kJ$

Hence, the standard Gibbs free energy of the reaction is 746.91 kJ

7 0

3 years ago