If a sample of 70.0 g of carbon oxide was reacted completely with 32.0 g of oxygen how many moles of carbon dioxide will be produced
Please answer it is greatly appreciated!

2.32 moles of carbon dioxide will be produced .

Step-by-step explanation:

Here we have , a sample of 70.0 g of carbon oxide was reacted completely with 32.0 g of oxygen. We need to find how many moles of carbon dioxide will be produced . Let's find out:

According to question , given equation of reaction is :

⇒

Now , Mass are given as :

According to reaction , 32 g of + 2(28 g of CO ) gives 2( 44 g of ) or ,

32 g of + 56 g of CO  gives 88 g of

So ,  32 g of + 70 g of CO  gives :

⇒

Moles of    =

Moles of    =

Therefore , 2.32 moles of carbon dioxide will be produced .

step-by-step explanation: given equation a = h(b 1+b 2)

also we are given values of a, h and b 1 as :

a = 16, h = 4, and b 1 = 3.

in order to solve it for b 2, we need to plug the given values of   a, h and b 1 .

therefore, plugging values of   a, h and b 1   in given equation, we get

16 = 4( 3 + b 2)

first dividing both sides by 4, we get

4 = 3 + b 2

subtracting 3 from both sides, we get

4 -3 = 3 -3 + b 2

1 = b 2.

it goes right