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3 years ago

15

Please please please help please

1 answer:

denpristay [2]3 years ago

3 0

Hydrogen and oxygen! Happy holidays btw

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Please help me thanks so much....I’ll mark you?!?!:))))

Marrrta [24]

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Explanation:

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3 years ago

Jordan needs to repeat the experiment but his teacher says that he needs to improve his design in his second experiment what sho

Margarita [4]

Just add more detail in the second experiment explain every little thing.

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3 years ago

Read 2 more answers

Equation 3x-5=-2x+ 10?<br> O<br> 0<br> x= 5<br> -5 = x<br> -15 = -5x<br> -5x = 15

Harman [31]

Answer:

are those the answer choice

7 0

3 years ago

6 CO2 + 12 H2O C6H12O6 + 6 H2O + 6 O2<br><br>how many hydrogen atoms are involved in this reaction?

Romashka-Z-Leto [24]

How many hydrogen atoms are involved in this reaction? 3

7 0

3 years ago

Calculate the mass of chromium metal produced when 425.0mL of 0.25M chromium(ll) nitrate reacts with a strip of zinc that remain

Reil [10]

The balanced chemical equation for the production of chromium metal from the reaction of chromium(ll) nitrate reacts with a strip of zinc is:

3 Zn + 2 Cr(NO₃)₃ → 2 Cr + 3 Zn(NO₃)₂

This is a redox reaction, which <u>is a chemical reaction in which one or more electrons are transferred between the reagents</u>, causing a change in their oxidation states. In the proposed reaction, Cr oxidation state goes from +3 to 0, becoming metallic chromium, while Zn goes from being Zn⁰ to Zn²⁺.

<u>The mass of chromium metal produced in the above reaction will be,</u>

425.0 mL x $\frac{1 L}{1000 mL}$ x $\frac{0.25 mol Cr(NO_{3})_{3} }{1 L}$ x $\frac{2 mol Cr }{2 mol Cr(NO_{3})_{3} }$ x $\frac{51.9961 g Cr}{1 mol Cr}$ = 5.52 g

So, the mass of chromium metal produced when 425.0mL of 0.25M chromium(ll) nitrate reacts with a strip of zinc that remains in excess is 5.52 g of Cr.

6 0

3 years ago