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Kobotan [32]
3 years ago
13

What is the electron configuration of a transition metal in block d

Chemistry
1 answer:
Bad White [126]3 years ago
4 0

Answer:

U gotta check ur book for that or Google maybe..

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The average rate of consumption of br− is 1.86×10−4 m/s over the first two minutes. what is the average rate of formation of br2
Scorpion4ik [409]
By considering the reaction equation is:
5Br(aq)+BrO3(aq)+6H(aq)= 3Br2(aq)+3H2O(l)
when the average rate of consumption of Br = 1.86x10^-4 m/s
So from the reaction equation 
5Br → 3Br2 when we measure the average rate of formation (X) during the same interval So,
∴ 1.86x10^-4/5 = X / 3
∴X = 1.1 x 10^-4 m/s
∴the average rate of formation of Br2 = 1.1x10^-4 m/s


7 0
3 years ago
Help please i give brainlist
shtirl [24]
The order of the answers are as follows:
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5 0
3 years ago
A ___ such as h20 is a symbol that shows the elements in a compound and the ratio of atoms
KATRIN_1 [288]
I think the answer is 15
4 0
3 years ago
Niven wants to calculate the mass of mgo that is produced by burning of 28.0g of mg. What is the first step in nivens calculatio
babymother [125]

Answer: -

The experiment Niven is doing is burning of Mg.

The first step would be finding the molar mass of MgO

Atomic mass of Mg = 24 g

Atomic mass of Oxygen = 16 g

Molar mass of MgO = 24 x 1 + 16 x 1 = 40 g

The balanced chemical equation for this reaction is

2 Mg + O2 -- > 2MgO

From the balanced equation we see that

2 Mg gives 2 MgO

2 x24 g of Mg O gives 2 x 40 g of MgO.

28g of MgO gives \frac{2 x 40 gram x 28 gram }{2 x 24 gram}

= 46.66 g of MgO.

8 0
3 years ago
Read 2 more answers
How many grams of hydrogen are needed to produce 1.80 g of water according to this equation? 2H2 + O2 → 2H2O
Arisa [49]

Hey there!:

Molar mass:

H2 = 2.01 g/mol    ;    H2O = 18.01

Given the reaction:

2 H2 + O2 = 2 H2O

2 * (2.01 ) g H2 ------------- 2 * ( 18.01 ) g H2O

mass H2 --------------------- 1.80 g H2O

mass H2 = 1.80 * 2 * 2.01 / 2* 18.01

mass H2 = 7.236 / 36.02

mass H2 = 0.2008 g


Hope that helps!

7 0
3 years ago
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