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And the number of nitrogen atoms is
Why use such an absurdly large number? Well, if we got
And thus we got..........
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From a consideration of the Lewis structure of the thiocyanate ion, SCN–, in which carbon has a double bond with both the sulfur and nitrogen atoms, what are the formal charges on the sulfur, carbon, and nitrogen atoms?
As is typical we put the least electronegative atom in the middle...and we gets Lewis structures of.... $N-=C-S^(-)$, else, $""^(-)N=C=S$. And thus the negative charge is conceived to lie on...
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Given 7 equiv calcium atoms; 10 equiv of carbon atoms; and 9 equiv of nitrogen atoms, how many equiv of $"calcium cyanide"$ could we make?
$"Calcium cyanide"$ is formulated by taking the calcium ion, $Ca^(2+)$, and binding it to 2 equiv of the cyanide ion, $""^(-):C-=N$. So for $7xxCa$, $10xxC$, and $9xxN$, at most...
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How do you write the equation for this reaction: Nitrogen gas and fluorine gas combine to produce nitrogen trifluoride gas?
$NF_3$ is in fact not so nasty .... it is much safer than $NCl_3$ or $NI_3$.. Of course the direct synthesis with fluorine gas is the province of specialist inorganic...
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A 1.50-g sample of nitrous oxide contains $2.05 * 10^22$ $N_2O$ molecules. How many nitrogen atoms are in this sample? How many nitrogen atoms are in 44.0 g of nitrous oxide?
Note: This answer may seem to be quite long, but that is because I have tried to explain each of the steps fully and clearly. If you want, you can...
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Which option contains a $2*g$ mass of sodium atoms....
$1.$ $5.24xx10^22*"sodium atoms?"$
$2.$ $6.022xx10^24*"sodium atoms?"$
$3.$ $3.12xx10^23*"sodium atoms?"$
$4.$ $5.24xx10^22*"sodium atoms?"$
We know that $1*mol$ contains $6.022xx10^23$ individual sodium atoms, and has a mass of $22.99*g$. And thus for $1.$ there is a $2*g$ mass of $Na$. For $2.$ there is...
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Under certain conditions of temperature and pressure, hydrogen gas and nitrogen gas react to form ammonia gas. Determine the mass of ammonia produced if 3.50 moles of hydrogen has reacts with 5.00 moles of nitrogen gas?
Start by balancing the equation for the reaction between hydrogen $"H"_2$ and nitrogen $"N"_2$, which produces ammonia $"NH"_3$: $color(darkgreen)(1) color(white)(.) "N"_2 (g) + color(darkgreen)(3) color(white)(.) "H"_2 to color(darkgreen)(2) color(white)(.) "NH"_3...
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Nitrogen (N) and hydrogen (H) react wth each other to produce ammonia ($NH_3$). This reactor is shown in an equation as $N_2 + 3H_2 -> 2NH_3$. What is the ratio of nitrogen atoms to hydrogen atoms in ammonia?
The chemical formula for ammonia is $2NH_3$ meaning that we have two nitrogen atoms and six hydrogen atoms. To find the ratio of nitrogen atoms to hydrogen atoms...
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Nitrogen gas (N2) reacts with hydrogen gas (H2) to form ammonia (NH3). At 200°C in a closed container, 1.05 atm of nitrogen gas is mixed with 2.02 atm of hydrogen gas. At equilibrium the total pressure is 2.02 atm. What is the partial pressure of hydrogen gas at equilibrium?
First, write the balanced chemical equation for the equilibrium and set up an ICE table. $color(white)(XXXXXX)"N"_2 color(white)(X)+color(white)(X)"3H"_2 color(white)(l)⇌ color(white)(l)"2NH"_3$ $"I/atm": color(white)(Xll)1.05 color(white)(XXXl)2.02 color(white)(XXXll)0$ $"C/atm": color(white)(X)-x color(white)(XXX)-3x color(white)(XX)+2x$ $"E/atm": color(white)(l)1.05- x...
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The total pressure is 600 mmHg after 0.50 moles of nitrogen gas, $N_2$, and 1.0 mole of nitrogen dioxide, $NO_2$, gas are mixed in a closed container. There is no reaction between the gases. What is the partial pressure of the nitrogen dioxide?
Old $"Dalton's Law of partial pressures"$ tells us that in a gaseous mixture, the exerted by a component gas is the same as the pressure it would exert if it...
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Which sample has the most number of atoms?
$A.$ $"1 mole of oxygen atoms;"$
$B.$ $"1 mole of oxygen molecules;"$
$C.$ $"1 mole of ozone molecules;"$
$D.$ $"Each sample contains the same number of atoms."$
Mass is a measure of the number of particles. Here you have $O$ atoms, and dioxygen, $O_2$, and ozone molecules, $O_3$ but each have the same mass by specification. There...
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